For a fixed mass of gas at a constant temperature, what happens to the vv-n,4th wv2yicy9yv 9olume if the pressure of t-2vyy4 99iv,h wctvn yhe gas is doubled?

  Which of the following conditions makes gases deviate from idealtog-rp: hji3+ behavior?

  Based on the graph below, choose2.mhtztz-t .gy yw-+ zypk 4d. the correct statement that describes the relationship between pressure and temperature for a fixed mass and volume of a gas-my 24p kth .-y. dzywtgztz+.?

  The ideal gas equation is a formula tha/eh t( yypp zy(n.pk94t combines the relationship between pressure, volume, temperature, and the numbe9/z. p4(ptk yy(hypn er of moles.
1.Complete the table below by calculating the missing variables of the ideal gas equation.

P	V	n	T
$\times10^4$Pa	$0.015m^3$	0.400mol	$37^{\circ}C$
152,000Pa	$m^3$	2.00mol	298.15K
31,000Pa	$0.25m^3$	mol	271.15K
250kPa	$0.75dm^3$	0.580m0l	k

2.A $256cm^3$ flask contains 0.800g of a gaseous compound with an empirical formula of CHCl. The pressure and the temperature of the gas are respectively $10^5$, Pa10 and 373K. Determine the molecular formula of the compound.

  Liquid butanol $(C_4H_9OH)$ burns or combusts in oxygen to produce $CO_{2(g)}$ and $H_2O$(g).
1.Write a balanced equation, including state symbols, for this reaction.
2.When $1.250cm^3$ of butanol is combusted in excess oxygen,$1.921dm^3$ of water vapor is collected at a pressure of 125.0 kPa and $150.0^{\circ}C$. Calculate the moles of butanol that were combusted.  mol
3.Determine the density of liquid butanol in $g\:cm^{-3}$.  g $cm^{-3}$

  Based on the table below, what is the correct calculation to determ- z4:fm;zo, h3y+oeoz9q06 z vcffkyaine the final volume of a am9oko yz0hf ;o+,yqfv3- ef 4:zzcz 6fixed mass of gas:

Initial	Final
Pressure = 1.00 atm	Pressure = 1.60 atm
Temperature =$20^{\circ}C$	Temperature =$10^{\circ}C$
Volume =$5.00dm^3$	Volume = ?

  Automobile airbags are infl bovkgq b: hb,op+40e6ated with $N_2$, a byproduct of sodium azide decomposition, according to the following reaction.
$2NaN_{3(s)}\rightarrow2 Na_{(s)}+3N^{2(g)}$
Calculate the mass (in grams) of sodium azide needed to generate $0.07m^3$ of $N^2$ at $1.01\times10^{5}Pa$ and $26.0^{\circ}C$.$n_{N2}$=  mol, mass of $NaN_3$=  g

  14.01g of nitrogen gas + ci xbdh,jk(yd1cx ,0$(N_2)$ is reacted with excess $H_2$. What volume of ammonia $(NH_3)$gas would be produced at STP? The molar volume of a gas at STP is $22.7dm^3$.
$N_{2(g)}+3H_{2(g)}\rightarrow2NH_{3(g)}$

  Sodium azide is an ionic compound found wivfol ;-jw / 96se rjrf+,dej/kthin the airbags of some older cars. The ae jlks/-jj v,;d/f9frwo +6e rirbag is deployed as a safety feature in the event of an accident. In this application, the sodium azide decomposes rapidly, and the gas formed inflates the airbag.
The decomposition of sodium azide under these conditions is given below.
$2NaN_{3(s)}\rightarrow2Na (s)+3 N_{2(g)}$
1.Suggest the formula and charge for the azide ion.
2.A typical airbag requires $65.0dm^3$of nitrogen gas for complete inflation at STP. Using section 2 of the data booklet, calculate the mass of sodium azide that the airbag must contain for this purpose.Molar mass for sodium azide calculated=  $g mol^{-1}$

  Which of the following gases most closely 79* 3i;tciww qf+ayeyaligns with the behavior of an ideal g9w;acey 7w*ity q+fi3as?

  Under which conditions would a gas deviate the most from tthl 1mf(49yc8 m6zql whe ideal gas model?

  A sample of gas at a certain temperature,ne f;rn0 hsh5d*2 b0jb pressure, and volume $(T_1,P_1,and V_1T)$ undergoes a change in temperature and pressure $(T_2andP_2)$.What is the new volume $(V_2)$?
Before: $T_1,P_1,V_1$;
After: $P_2=2P_1$ AND $T_2=\frac{1}{2}T_1$